For a hypothetical reaction, the activation energy is E_act = 50.2 kJ/mol and it has an Arrhenius constant of 22.3 M^-1s^-1. Determine what the rate constant would be if the temperature was 400$\degree$C.

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The Answer of For a hypothetical reaction, the activation energy is E_act = 50.2 kJ/mol and it has an Arrhenius constant of 22.3 M^-1s^-1. Determine what the rate constant would be if the temperature was 400$\degree$C.

For a Hypothetical Reaction, the Activation Energy Is Eact = °\degree°

For a Hypothetical Reaction, the Activation Energy Is E_act = $\degree$